JEE Main · 2026 · 22 Jan 2026 · Shift 2 · Chemical Kinetics

The Boltzmann factor $e^{-E_a/RT}$ gives the fraction of molecules whose energy is equal to or greater than $E_a$, not less than it, so statement (A) is wrong. A smaller activation energy makes $e^{-E_a/RT}$ larger and the reaction faster at a fixed temperature, so statement (B) is correct, and the empirical temperature coefficient means a rise of about $10^{\circ }\mathrm{C}$ roughly doubles the rate, so statement (C) is correct. A plot of $\log k$ against $1/T$ is a straight line of slope $-\frac{E_a}{2.303R}$, not $-\frac{E_a}{R}$, so statement (D) is wrong. The correct statements are B and C only.